1. The molarity of the stock solution is 1.26 M
2. The molarity of the diluted solution is 0.126 M
<h3>1. How to determine the molarity of stock solution </h3>
From the question given above, the following data were obtained
- Mole of KIO₃ = 6.05 mole
- Volume = 4.8 L
- Molarity of stock solution =?
Molarity = mole / Volume
Molarity of stock solution = 6.05 / 4.8
Molarity of stock solution = 1.26 M
<h3>2. How to determine the molarity of the diluted solution </h3>
- Molarity of stock solution (M₁) = 1.26 M
- Volume of stock solution (V₁) = 10 mL
- Volume of diluted solution (V₂) = 100 mL
- Molarity of diluted solution (M₂) =?
M₁V₁ = M₂V₂
1.26 × 10 = M₂ × 100
12.6 = M₂ × 100
Divide both side by 100
M₂ = 12.6 / 100
M₂ = 0.126 M
Complete question
An aqueous potassium iodate stock solution is made by dissolving 6.05 mol KIO3 in sufficient water for the final volume of the solution to be 4.80 L.
Calculate the molarity of the stock KIO3 solution.
A 10.0 mL aliquot is removed from the described stock solution and diluted to a total volume of 100.0 mL.
Calculate the molarity of the dilute solution
Learn more about dilution:
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I haven’t see anything like that
Answer:
lol no. They are still frogs but you probaly not do that. lol
Explanation:
